Tech Chemistry Final Exam Review Guide



Chemistry Final Exam Review Guide Name __________________

1. Place the following prefixes in order from largest to smallest:

Deci- hecta- milli- kilo- ones deca- centi-

5 2 7 1 4 3 6

2. Make the following conversions:

765 m = ___765000________ mm

4.67 km = ___.00467________ m

56.98 mm = ____.0005698_____ hm

3. Complete the following chart for the metric system.

|Measurement |Equipment |Units |

|Volume |Graduated cylinder |Ml or cm3 |

|Mass |Balance |Grams |

|Time |Stopwatch |Seconds |

|Length |Meter stick |Meters |

|Temperature |Thermometer |Kelvin |

4. Define accuracy. Hitting the bulls eye. The correctness of the measurement compared to the true or accepted value.

5. Define precision. Hitting the same wrong spot over and over. When values agree with each other

6. Identify the following as qualitative or quantitative.

___Qual____ red _____Quant__ 150 pounds

___Qual____ smelly _____Qual___ cold

___Quant___ 55 mph ______Quant_ 15 grams

7. What piece of equipment changes vapor to liquid in the distillation process? Condenser

8. What pieces of equipment are needed in filtration? What is the liquid called collected from the filtration process? Funnel and filter paper, liquid is called the filtrate

9. Name three other separation techniques.

Crystallization, Chromatography, Distillation, Filtration, Decanting

10. What is the formula for density? What are the units for density? What equipment is needed in the lab to determine density?

D = m/V Units are g/mL or g/cm3 you need a balance and a graduated cylinder or ruler.

11. Rank the following densities from heaviest (bottom of a graduated cylinder) to lightest (top of a graduated cylinder): 1.4 g/mL, 3.7 g/mL, 0.05 g/mL, 5.9 g/mL, 8.5 g/mL, 2.6 g/mL. 8.5, 5.9, 3.7, 2.6, 1.4, .05

12. Determine if the following are physical or chemical properties or changes.

Milk sours __C______________ solubility _______P_____________

Evaporation __P_____________ iron rusting ______C____________

Grass growing _C_____________ boiling point _____P_____________

Reacts with acid __C___________ density __________P____________

Luster ______P______________ combustion ________C___________

13. What is the difference between an element, ion and a compound? Give an example of each. Element is a pure substance on periodic table, ion is a charged particle, compound is two or more elements chemically combined. Na, Na1+, NaCl

14. What is the difference between heterogeneous and homogeneous?

Heterogeneous is a solution that has layers, is not the same throughout (oil-water), Homogeneous is a solution that is the same at the top middle and bottom (kool-aid)

15. Determine if the following is a substance(you can write a formula) or a mixture.

Chlorine _____Substance_ Pure air _Homogeneous mixture_____________

Soil Heterogeneous mixture Water _Substance__________________

Carbon dioxide ___Substance Sugar water ___Homogeneous mixture_________

16. Distinguish the difference between the following sets of words:

molecule and element: Two or more elements chemically combined/Smallest part of matter and on the periodic table.

colloid , precipitate and solution: + tyndall effect (tunnel of light), insoluble solid formed, mixture of a solute and a solvent.

mixture and suspension: physical mixture of two or more substances, heterogeneous mixture of usually a solid suspended in a liquid.

solvent and solute : thing doing the dissolving, thing getting dissolved

dependent and independent variable: DRY MIX. Dependent is the responding variable on the Y axis, Independent is the manipulated variable on the X axis.

symbol, subscript, formula and equation Mg + O2 ( MgO Mg is a symbol, 2 is a subscript, MgO is a formula and the equation is reactants yield products. So Mg + O2 are reactants and MgO is the product. The arrow is the yield.

17. What is an alloy? Give an example of an alloy. Is it homogeneous or heterogeneous.

A homogeneous mixture of two or more solids

18. Use the following chart to determine the identity of the mixtures as solution, colloid, or suspension.

|Mixture 1 |Negative Tyndall Effect |No sediment |Clear liquid |

|Mixture 2 |Negative Tyndall Effect |Has sediment at the bottom of the |Clear liquid |

| | |beaker | |

|Mixture 3 |Positive Tyndall Effect |Has sediment suspended in beaker |Cloudy liquid |

Mixture 1 __Solution___________ Mixture 2 __Suspension__________

Mixture 3 ___Colloid and Suspension__________________

19. If a brick has a 2cm X 4cm X 3 cm dimension what is its volume? _24 cm3__________

20. Determine the density of the following.

A. A metal has a mass of 25.0 g and a volume of 500 mL. What is it’s density? Will with metal float or sink in water? __.05 g/mL, float______________

B. A liquid has a density of 2.6 g/mL and a mass of 5000.0 g, what is it’s volume? _1923.1 mL_________

C. A rock has a mass of 0.30 g and when placed in a graduated cylinder the volume of water started at 10.0ml and rose to a volume of 55.0 ml. What is the density? .3/45 = .007 g/mL

D. A 40.0 g cube has one side with a length of 2 cm, what is it’s density? _2x2x2=8 cm3__so 40.0g/8 cm3 = 5 g/cm3____________

21. Complete the following:

|Subatomic Particle |Charge |Where Located |

|Proton |+ |Nucleus |

|Neutron |Neutral |Nucleus |

|Electron |- |Outside nucleus |

22. In a neutral atom the number of protons = ___electrons___ = __Atomic number____

23. Atomic Mass = __Protons_____ + _Neutrons_______________________

24. What is the name of the subatomic particle that determines the identity of the atom?Proton

25. What is the name for a negative ion? Did the atom gain or lose an electron to become a negative ion? Is this a metal or a non metal? What is the name for a positive ion?

Anion, gained, non metal, Cation

26. Complete the electron dot structures for the following elements:

4 5 1 2

C N K He

27. Give the oxidation states (charges) for the following:

Mg Al Br O

28. Complete the following chart:

|Substance |Symbol |Atomic Number |Mass Number |Number of Protons |Number of Neutrons |Number of Electrons |

|Calcium |Ca |20 |40 |20 |20 |20 |

|Chlorine |Cl |17 |35 |17 |18 |17 |

|Zinc |Zn |30 |65 |30 |35 |30 |

|Krypton |Kr |36 |84 |36 |48 |36 |

|Magnesium-28 |Mg |12 |24 |12 |12 |12 |

29. List four properties of metals.

Shiny, malleable, conductor, reacts with acids, lose electrons, elements are smaller than the ions.

30. Where are metals found in the periodic table? Where are the most active metals found?

Left, bottom right (Fr)

31. List the four properties of nonmetals.

Dull, brittle, insulators, gain electrons, elements are larger than the ions.

32. Where are nonmetals found in the periodic table? Where are the most active nonmetals?

Right, upper halogens (F)

33. Give an example of a metalloid. ___Silicon__________

34. Elements in the same _group________ have similar properties. Name an element that has properties similar to Oxygen. ___Selenium___________

35. Sketch a periodic table and label the following:

Groups/families Periods/rows Halogens Chalcogens

Noble gases Alkali Metals Alkaline earth metals Transitional metals

Lanthanides Actinides Metalloids Groups 1-18

36. What is an isotope? Which subatomic particle would be different if the atom is an isotope?

Atoms of the same element with different atomic mass due to neutrons

37. What three things did Rutherford conclude from his gold foil experiment about atoms?

Atom is mostly empty space, nucleus is very dense and the nucleus has a + charge

38. Match the following.

__B___ Arranged the periodic table by atomic mass a. Moseley

__C___ Based the periodic table on the law of octaves b. Mendeleev

__A___ Arranged the periodic table by increasing atomic number c. Newland

39. What is the periodic trend for atomic radius? Which has a larger atomic radius Potassium or Calcium?_K____________ Sodium or Lithium? ___Na________

Decrease going across

Increase going down

40. What is the periodic trend for ionization energy? What is ionization energy? Which has the larger ionization energy Sodium or Chlorine? __Cl_______________

Increase going across Energy require to remove an electron

Decrease going down

41. What has a higher electronegativity? Metals or Nonmetals What is the trend? Which has the larger electronegativity Francium or Fluorine? F

Increase going across

Ability of an atom to attract an electron

Decrease going down

42. Using the following Group numbers, what is the charge an ion in that group usually has?

|Group 1 |Group 2 |Group 13 |Group 14 |Group 15 |Group 16 |Group 17 |Group 18 |

|1+ |2+ |3+ |4+/- |3- |2- |1- |0 |

43. If an ion has a charge of 2+, did it gain or lose electrons? lost

44. If an ion has a charge of 3-, did it gain or lose electrons? gained

45. What type of bond is formed when electrons are transferred between two atoms? Ionic

46. What type of bond is formed when electrons are shared between two atoms? Covalent

47. What type of covalent bond is formed when electrons are shared equally? Non polar covalent

48. What type of bond is formed with oppositely charged ions? Ionic

49. How many atoms of calcium, phosphorus, and oxygen are in the molecule Ca3(PO4)2?

Calcium-3, Phosphorus-2, Oxygen-8

50. Write the chemical formula for the following ions and then name the item.

Na+ and Cl - ___NaCl_____________________

Al3+ and OH- ____Al (OH) 3___________________

K+ and PO4 3- ___K3PO4____________________

Mg 2+ and CO3 2- __MgCO3____________________

51. Name the following or write the formula

KOH _Potassium hydroxide Manganese IV chloride ____MnCl4_

Ca3N2 _Calcium nitride___ Lithium oxide ___Li2O__

Mg3(PO4)2 Magnesium phosphate__Beryllium fluoride _BeF2____

LiCl _Lithium chloride____ Carbon tetrachloride __CCl4____

SnCl2 Tin II Chloride_________ Sodium hypochlorite ___NaClO___

SO3 ___Sulfur trioxide________ Calcium nitrate __Ca(NO3)2____

Name the following acid HNO3 ___Nitric Acid_______________________

52. Name the three types of radiation and give the symbols and what they are stopped by.

|Type of radiation |Symbol and charge |Energy level |Stopped by |

|Alpha |4 |Low |Paper |

| |He | | |

| |2 | | |

|Beta |0 |Medium |Aluminum Foil |

| |E | | |

| |-1 | | |

|Gamma |Pure energy |High |1 inch of lead |

53. Which process produces all elements heavier than Helium? Fission or Fusion

54. Complete the following half life equations:

a. Francium-226 undergoes alpha decay:

226 4 222

__Fr He At

87_____ ( 2_______ + _____85___

b. Sulfur-33 undergoes beta decay

33 0 33

S E Cl

16______ ( ___-1__ + ____17___

55. Name the following covalent compounds.

CO _Carbon monoxide__________ P2O5 _Diphosphorus pentaoxide__________

CCl4 Carbon tetrachloride________ N2O4 _Dinitrogen tetraoxide____________

List the Greek Prefixes: 1 – 10 mono-1, di-2, tri-3, tetra-4, penta-5, hexa-6, hepta-7, octa-8, nona-9, deca-10

56. Write the formula for water. H2OWhat is the name given to the lower case two?subscript

57. Complete the following chart

| |Protons |Neutrons |Electrons |Oxidation # |Gain or Lose |Metal or Nonmetal |

| | | | | |electrons | |

| |11 |13 |10 |1+ |Lost 1 |metal |

|Sodium-24 | | | | | | |

| |16 |16 |18 |2- |Gained 2 |nonmetal |

|Sulfur | | | | | | |

58. How many electrons are needed to satisfy the octet rule? __8___________

59. What piece of equipment is needed to test for ions? conductivity meter_______

60. Balance and give the type of reaction in each of the following.

2HgO ( 2Hg + O2 _Decomposition__________

NaCl + AgNO3 ( NaNO3 + AgCl _Double Displacement_____

Mg +2 HCl ( MgCl2 + H2 _Single Displacement______

2Mg + O2 -> 2MgO _Synthesis_______________

NaOH + HCl ( NaCl + H2O _Double Displacement______

61. Using the Law of Conservation, explain why the products must equal the reactants in a chemical equation. Label the products and reactants. Balance the reaction. Underline the coefficient and circle the subscripts.

Example:

Sun + 6CO2 + 6 H2O ( C6H12O6 + 6 O2 subscript is the 2

Reactants Products

Law of Conservation states you cannot create or destroy matter so if the reactants equal 100 g then the products must also add up to 100g.

62. How many energy levels are on the periodic table? How many electrons can locate in energy levels 1,2,and 3? 7 levels on the periodic table, 2 in the first,8 in the second, 18 in the third level.

63. Construct a Bohr model for the following elements. Circle your choice to determine if the element would like to lose or gain electrons to be stable.

1s22s22p63s1 Lose or gain__lost 1__ electrons.

Na )2 )8 )1

1s22s22p5 Lose or gain __gained 1__ electrons.

F )2 )7

1s22s22p4 Lose or gain _gained 2__ electrons.

O )2 )6

64. What is the boiling point of water? __1000 C______________

65. What is the freezing point of water? __0 0 C______________

66. Give the three states of matter and tell the shape(definite or not definite), volume and energy of each. State of matter Shape Volume Energy

Solid definite definite low

Liquid indefinite definite medium

Gas indefinite indefinite high

67. Give the state of matter

__SOLID__ Definite shape and volume

__GAS___ No shape and takes the volume of the entire container

__LIQUID_ No shape but definite volume

__SOLID__ Low kinetic energy

__GAS___ High kinetic energy

__SOLID__ Rigid shape with vibrating molecules

__GAS ___ Free moving molecules

68. When snow melts the energy is absorbed/released and the overall reaction is endothermic/exothermic? ABSORBED/ENDOTHERMIC

69. When combustion occurs the energy is absorbed/release and the overall reaction is endothermic/exothermic? RELEASED / EXOTHERMIC

70. Which has more energy red lights or blue lights? (think about the spectrum)

BLUE

71. Which is more damaging UV waves or radio waves?

UV WAVES

72. Refer to read a heating curve below to answer the following questions:

What is occurring at number 1 __Solid is melting or freezing______

What is occurring at number 2 __Melting point or freezing point_______

What is occurring at number 3 ___Liquid is warming or cooling_________________

What is occurring at number 4 ___Boiling or Condensing______

What is the freezing point of this substance _0 degrees celcius_____

What is the boiling point of this substance ____100 degrees celcius_____

What is the melting point of this substance ____0 degrees celcius______________

Where is there a change in kinetic energy ___Stages 1 , 3, and 5 ____________

What state of matter has the highest molecular motion? __GAS__

What state of matter has the lowest molecular motion? ___SOLID__

As a solid melts does the molecular motion increase or decrease? _INCREASES__

As a liquid freezes does the molecular motion increase or decrease? _DECREASES_

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73. What is the state of matter of the noble gasses? ___GAS____

74. What is the only metal that is a liquid at room temperature? _Hg Mercury__

75. What is the state of matter of most metals? ___SOLIDS____

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Na

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